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Kinetic molecular theory

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slideshare about kinetic molecular theory....it was a reporrt in my pysical science subject.

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Kinetic molecular theory

  1. 1. KINETIC MOLECULAR THEORY
  2. 2. Democritus “matter was empty space filled with tremendous numbers of tiny particles called ATOMS” 5th century BC Aristotle did not support Democritus’ theory on molecules. 1600’S Some scientist support the theory and some evidences on small particles and the space around them sprouted. 1700’s
  3. 3. ATOMS One of the smallest parts that any substance can be divided into,that combines with other atoms that make a MOLECULE.
  4. 4. Pure substances Elements  A simple chemical substance compose of single atom  E.g. hydrogen(H) oxygen (O) carbon (C) Compound  Something that consist of a combination of two or more atoms  E.g. Water (H₂O) a combination of hydrogen and oxygen
  5. 5. molecules  The smallest unit into which any substance can be divided without losing its own chemical nature.  E.g. Gold* *even if a gold is broken into two, they are still golds.
  6. 6. Molecules Interact Cohesion  Attractive force between same kind of molecules. Adhesion  The ability where one kind of molecule attracts and clings to a different kind of molecule.
  7. 7. PHASES OF MATTER solid liquid gas
  8. 8. Solid Have definite shape and volumes. Molecules have fixed distances apart and bound by strong cohesive forces.
  9. 9. Liquids Molecules of a liquid are close together and bound by a cohesive force that are not as strong as in a solid.
  10. 10. Gases Composed of molecules with weak cohesive forces, no fixed shapes and no fixed volume.
  11. 11. SOLID LIQUID GAS SHAPE fixed variable variable VOLUME fixed fixed variable
  12. 12. Vapor- used to describe a gas that is in a liquid state. e.g. Evaporated water from the sea
  13. 13. Plasma*- Occur at extremely high temperature and are made up of charged part of atoms. *rare phase of matter
  14. 14.  At higher temperature, the molecules of a substance move faster with increased agitation and then they move a little faster apart thus expanding the substance. As the substance cools down, the motion slows and the molecular forces are able to pull the molecules closer together.
  15. 15.  Temperature of a gas is proportional to the average kinetic energy of the gas molecule.(e.g. ammonia molecules have greater average velocity at a higher temperature and a slower average velocity at lower temperature)  Kinetic energy involves the mass of the molecules as their velocity: ( KE = ½ mv² )- ( d= gt²/2 )
  16. 16. Thank you!!!!!!!!!!!!!!! Submitted by: CHRISTINE P.ORIA Bachelor of Science in Home Technology Education

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